Answer:
Molarity = 1.93 mol.L⁻¹
Explanation:
Molarity is the unit of concentration used to specify the amount of solute in given amount of solution. It is expressed as,
Molarity = Moles / Volume of Solution ----- (1)
Data Given;
Mass = 11.3 g
Volume = 100 mL = 0.10 L
First calculate Moles for given mass as,
Moles = Mass / M.mass
Moles = 11.3 g / 58.44 g.mol⁻¹
Moles = 0.1933 mol
Now, putting value of Moles and Volume in eq. 1,
Molarity = 0.1933 mol ÷ 0.10 L
Molarity = 1.93 mol.L⁻¹
Answer:
The new pressure is 1,65 atm
Explanation:
We use the gas formula, which results from the combination of the Boyle, Charles and Gay-Lussac laws. According to which at a constant mass, temperature, pressure and volume vary, keeping constant PV / T.
(P1xV1)/T1= (P2xV2)/T2
(1,23atmx 8,46L)/267 K = (P2 x 6,98L)/ 295K
0,039 atmx L/K = (P2 x 6,98L)/ 295K
P2=(0,039 atmx L/K)x 295K/6,98L =1,65 atm
Answer:
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Explanation:
Answer:
6.1×10^8
Explanation:
The reaction is;
Sn^2+(aq) + Cd(s) -----> Sn(s) + Cd^2+(aq)
E°cell = E°cathode - E°anode
E°cathode= -0.14 V
E°anode= -0.40 V
E°cell = -0.14-(-0.40)
E°cell= -0.14+0.40
E°cell= 0.26 V
But
E°cell= 0.0592/n log K
E°cell= 0.0592/2 log K
0.26= 0.0296log K
log K = 0.26/0.0296
log K= 8.7838
K= Antilog (8.7838)
K= 6.1×10^8
Answer:
you sure it is the right sign your using
